I II III IV V

Types of Chemical Reactions

Ch. 8 – Chemical Reactions

Describing Chemical Reactions

Evidence of a chemical change… Production of heat and light Formation of a gas Formation of a precipitate, a solid

product. Color change

Describing Chemical Reactions

A+B ABREACTANTS PRODUCTS

Describing Chemical Reactions

A. Combination / Synthesis (marriage) the combination of 2 or more

substances to form a compound

only one product

A + B AB

Mg(s) + O2(g) MgO(s)

A. Combination / Synthesis

Product: Must be a compound

B. Decomposition (divorce)

a compound breaks down into 2 or more simpler substances

only one reactant

AB A + B

H2O2 (aq)

B. Decomposition

Products: Can be elements or compounds

H2O(l) + O2(g)

C. Single Replacement (affair) one element replaces another in a

compound Metal replaces metal Nonmetal replaces nonmetal

A + BC B + AC

Zn(s) + HCl(aq)

C. Single Replacement

H2(g) + ZnCl2(aq)

AB + CD AD + CB

D. Double Replacement (Jerry Springer)

ions in two compounds “change partners” cation of one compound combines with

anion of the other

Pb(NO3)2(aq)+ NaI(aq) PbI2(s)+ NaNO3(aq)

D. Double Replacement

Products: Are compounds Sometimes one of the products is water

E. Combustion

the burning of a hydrocarbon to produce heat

CxHy + O2 CO2 + H2O

E. Combustion

Products:

During complete combustion theproducts are CO2 + H2O

C12H22O11 + 3O2 9C + 3CO2 + H2O

Warm up (practice)

Title: Reaction Types

Number Page (1-5)

1.

2.

3.

4.

5.

1.

Cu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s)

Single Replacement

2.

2 H2O(l) 2 H2(g) + O2(g)

Decomposition

3.

H2(g) + Cl2(g) 2 HCl(g)

Combination / Synthesis

4.

Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(s) + 2KNO3(aq)

Double Replacement

5. Combustion

C2H6 + O2 CO2 + H2O